• Chemistry Question?

    Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 1.80 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 865 mmHg . Identify the limiting reactant and determine the theoretical yield of ClF3 in grams.
    Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 1.80 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 865 mmHg . Identify the limiting reactant and determine the theoretical yield of ClF3 in grams.
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    Find the ratio of effusion rates of helium gas and xenon gas. Express your answer to three significant digits.
    Find the ratio of effusion rates of helium gas and xenon gas. Express your answer to three significant digits.
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    A sample of an unknown gas requires 45 seconds to effuse from a container. Under identical conditions, a sample of bromine gas effuses in 90 seconds. You know the unknown gas must have come from a gas tank in your lab. What is the identity of the unknown gas?
    A sample of an unknown gas requires 45 seconds to effuse from a container. Under identical conditions, a sample of bromine gas effuses in 90 seconds. You know the unknown gas must have come from a gas tank in your lab. What is the identity of the unknown gas?
    2 answers · Chemistry · 1 month ago
  • Chemistry Question?

    A gas mixture contains 1.24 g N2 and 0.95 g O2 in a 1.65-L container at 17 ∘C. Just need help on the partial pressure part Calculate the mole fraction of N2 - .599 Calculate the mole fraction of O2 - .40 Calculate the partial pressure of N2 Calculate the partial pressure of O2
    A gas mixture contains 1.24 g N2 and 0.95 g O2 in a 1.65-L container at 17 ∘C. Just need help on the partial pressure part Calculate the mole fraction of N2 - .599 Calculate the mole fraction of O2 - .40 Calculate the partial pressure of N2 Calculate the partial pressure of O2
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    A common way to make hydrogen gas in the laboratory is to place a metal such as zinc in hydrochloric acid (see the figure). The hydrochloric acid reacts with the metal to produce hydrogen gas, which is then collected over water. Suppose a student carries out this reaction and collects a total of 144.0 mL of gas at a pressure of 744 mmHg and a... show more
    A common way to make hydrogen gas in the laboratory is to place a metal such as zinc in hydrochloric acid (see the figure). The hydrochloric acid reacts with the metal to produce hydrogen gas, which is then collected over water. Suppose a student carries out this reaction and collects a total of 144.0 mL of gas at a pressure of 744 mmHg and a temperature of 25∘C. What mass of hydrogen gas (in mg) does the student collect? (The vapor pressure of water is 23.78 mmHg at 25∘C.)
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    The air in a bicycle tire is bubbled through water and collected at 25 ∘C. If the total volume of gas collected is 5.30 L at a temperature of 25 ∘C and a pressure of 761 torr, how many moles of gas was in the bicycle tire?
    The air in a bicycle tire is bubbled through water and collected at 25 ∘C. If the total volume of gas collected is 5.30 L at a temperature of 25 ∘C and a pressure of 761 torr, how many moles of gas was in the bicycle tire?
    2 answers · Chemistry · 1 month ago
  • Chemistry Question?

    A gas mixture contains 1.24 g N2 and 0.95 g O2 in a 1.65-L container at 17 ∘C. Calculate the mole fraction of N2 Calculate the mole fraction of O2 Calculate the partial pressure of N2 Calculate the partial pressure of O2
    A gas mixture contains 1.24 g N2 and 0.95 g O2 in a 1.65-L container at 17 ∘C. Calculate the mole fraction of N2 Calculate the mole fraction of O2 Calculate the partial pressure of N2 Calculate the partial pressure of O2
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    Calculate the root mean square velocity of I2(g) at 377 K. 19.1 m/s 192 m/s 6.09 m/s 101 m/s
    Calculate the root mean square velocity of I2(g) at 377 K. 19.1 m/s 192 m/s 6.09 m/s 101 m/s
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    The mass of a sample of gas is 944 mg. Its volume is 0.270 L at a temperature of 88∘C and a pressure of 975 mmHg. Find its molar mass.
    The mass of a sample of gas is 944 mg. Its volume is 0.270 L at a temperature of 88∘C and a pressure of 975 mmHg. Find its molar mass.
    1 answer · Chemistry · 1 month ago
  • Chemistry Question?

    What is the pressure in a 10.0-L cylinder filled with 0.465 mol of nitrogen gas at a temperature of 318 K ?
    What is the pressure in a 10.0-L cylinder filled with 0.465 mol of nitrogen gas at a temperature of 318 K ?
    2 answers · Chemistry · 2 months ago
  • Chemistry Question?

    What is the pressure in a 10.0-L cylinder filled with 0.465 mol of nitrogen gas at a temperature of 318 K ?
    What is the pressure in a 10.0-L cylinder filled with 0.465 mol of nitrogen gas at a temperature of 318 K ?
    1 answer · Chemistry · 2 months ago
  • Chemistry Question?

    Calculate the heat of atomization of C2HCl3, using the average bond energies in the following table: Bond Bond energy (kJ/mol) C−C 347 C=C 611 C≡C 837 H−C 414 C−Cl 339 H−Cl 431
    Calculate the heat of atomization of C2HCl3, using the average bond energies in the following table: Bond Bond energy (kJ/mol) C−C 347 C=C 611 C≡C 837 H−C 414 C−Cl 339 H−Cl 431
    1 answer · Chemistry · 2 months ago
  • Chemistry Question?

    ΔH∘rxn =-1648.4 kJ Calculate how much heat (in kilojoules) a hand warmer containing 18.0 g of iron powder produces.
    ΔH∘rxn =-1648.4 kJ Calculate how much heat (in kilojoules) a hand warmer containing 18.0 g of iron powder produces.
    1 answer · Chemistry · 2 months ago
  • Chemistry Help Please?

    Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ
    Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ
    1 answer · Chemistry · 2 months ago
  • Chemistry Question?

    The standard enthalpy of formation for ethanol [CH3COOH(l)] is −484.3 kJ/mol. What is the correct formation equation corresponding to this ΔHof? 2C(s,graphite)+2H2O(g)→CH3COOH(l) 2C(s,graphite)+2H2(l)+O2(l)→CH3COOH(l) 2C(s,graphite)+2H2(g)+O2(g)→CH3COOH(l) 2C(s,graphite)+2H2O(l)→CH3COOH(l)
    The standard enthalpy of formation for ethanol [CH3COOH(l)] is −484.3 kJ/mol. What is the correct formation equation corresponding to this ΔHof? 2C(s,graphite)+2H2O(g)→CH3COOH(l) 2C(s,graphite)+2H2(l)+O2(l)→CH3COOH(l) 2C(s,graphite)+2H2(g)+O2(g)→CH3COOH(l) 2C(s,graphite)+2H2O(l)→CH3COOH(l)
    1 answer · Chemistry · 2 months ago
  • Chemistry Question Help Please?

    When 1.557 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 26.31 ∘C to 38.29 ∘C. Find ΔErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.81 kJ/∘C.
    When 1.557 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 26.31 ∘C to 38.29 ∘C. Find ΔErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.81 kJ/∘C.
    1 answer · Chemistry · 2 months ago
  • Chemistry Question?

    A cylinder equipped with a piston expands against an external pressure of 1.50 atm . If the initial volume is 0.550 L and the final volume is 1.300 L , how much work (in J) is done?
    A cylinder equipped with a piston expands against an external pressure of 1.50 atm . If the initial volume is 0.550 L and the final volume is 1.300 L , how much work (in J) is done?
    1 answer · Chemistry · 2 months ago
  • Chemistry Question Help?

    Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g... ΔHorxn = -1418 kJ How much heat is produced by the complete reaction of 7.44 kg of nitromethane?
    Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g... ΔHorxn = -1418 kJ How much heat is produced by the complete reaction of 7.44 kg of nitromethane?
    1 answer · Chemistry · 2 months ago
  • Cant get the right answer to a chemistry question?

    A block of copper of unknown mass has an initial temperature of 65.6 ∘C. The copper is immersed in a beaker containing 92.7 g of water at 22.6 ∘C. When the two substances reach thermal equilibrium, the final temperature is 24.5 ∘C. What is the mass of the copper block? Assume that Cs,H2O=4.18J/(g⋅∘C) and Cs,Cu=0.385J/(g⋅∘C). I keep getting 35.1 g... show more
    A block of copper of unknown mass has an initial temperature of 65.6 ∘C. The copper is immersed in a beaker containing 92.7 g of water at 22.6 ∘C. When the two substances reach thermal equilibrium, the final temperature is 24.5 ∘C. What is the mass of the copper block? Assume that Cs,H2O=4.18J/(g⋅∘C) and Cs,Cu=0.385J/(g⋅∘C). I keep getting 35.1 g but its not right
    2 answers · Chemistry · 2 months ago
  • Chemistry Question?

    s the burning of nitrogen to nitrogen(II) oxide exothermic or endothermic? What is the sign of the energy change?
    s the burning of nitrogen to nitrogen(II) oxide exothermic or endothermic? What is the sign of the energy change?
    2 answers · Chemistry · 2 months ago