Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Stoichiometry
Gas Laws
1. What volume of O¬2(g) is consumed in the combustion of 50.0 L of butane (C4H10) if both gases are measured at STP?
1 answer
figure the moles
multiply by 22.4L/mole
You can
ask a new question
or
answer this question
.
Related Questions
How many grams of Butane (C4H10) must be burned to release 6375 KJ of heat?
Given: Molar mass of C4H10 =
how many moles of water vapour are formed when 10 liters of butane gas C4H10 is burned in oxygen at stp?
Many cigarette lighters contain liquid butane, C4H10(l). Using standard enthalpies of formation, calculate the quantity of heat
Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete
What will be the change in enthalpy when 100.0 g of butane, C4H10, is burned in oxygen as shown in the thermochemical equation
how many moles of butane gas c4h10 react to produce 3.50moles of water?
How many moles of water are produced when 0.48 moles of butane c4h10 react?
The enthalpy of combustion of butane C4H10 is described by the reaction:
C4H10(g) + (13/2) O2(g) -> 4CO2(g) + 5H2O(g) ΔH°rxn =
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.4 C. A 250 mL sealed flask contains
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mole and a normal boiling point of -0.4 C. A 250 mL sealed flask contains