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18 Nov 2019
Please show work and all parts. Thanks!
Nitromethane CH3NO2, is burned as a fuel; the (unbalanced) equation for the reaction is CH3NO2 (l) + O2 (g) rightarrow CO2 (g) + N2 (g) + H2O (g) The standard enthalpy charge of the reaction for the balanced reaction. with the lowest whole number coefficients is -1288.5 kJ. If the of CO2 (g) = -393.5 kj/mol and the of H2O (g) = 242 kJ/mol calculate for . A sample of nitromethane is scaled in a 15.0 L flask with oxygen gas, in the stoichiometric ratio indicated in the balanced equation above. The flask is heated to 100 degree C and the reaction is then allowed to go to 100% completion. If the total pressure of all gases in the flask at 100 degree C is 950 torr when the reaction is complete, what was the mass of nitromethane sample used?
Please show work and all parts. Thanks!
Nitromethane CH3NO2, is burned as a fuel; the (unbalanced) equation for the reaction is CH3NO2 (l) + O2 (g) rightarrow CO2 (g) + N2 (g) + H2O (g) The standard enthalpy charge of the reaction for the balanced reaction. with the lowest whole number coefficients is -1288.5 kJ. If the of CO2 (g) = -393.5 kj/mol and the of H2O (g) = 242 kJ/mol calculate for . A sample of nitromethane is scaled in a 15.0 L flask with oxygen gas, in the stoichiometric ratio indicated in the balanced equation above. The flask is heated to 100 degree C and the reaction is then allowed to go to 100% completion. If the total pressure of all gases in the flask at 100 degree C is 950 torr when the reaction is complete, what was the mass of nitromethane sample used?
Keith LeannonLv2
22 Apr 2019