Answer: 4/3
Proof:
The numerator of the answer will be the number of molecules of H2O, which is 4.
The denominator will be the number of molecules of CO2, which is 3.
Since both molecules are products, the fraction will be positive.
For the following reaction, to get the rate of formation of H2O, what must we multiply the rate of formation of CO2 by?
For the following reaction, to get the rate of formation of H2O, what must we multiply the rate of consumption of O2 by? 4NH3+5O2→4NO+6H2O Report your answer as a fraction.
1)For the following reaction, to get the rate of formation of SiO2, what must we multiply the rate of formation of H2O by? 2Si2H2+5O2⟶4SiO2+2H2O 1/2 2 −1/2 −2 2)For the following reaction, if O2 is used up at a rate of 4.42Mhr, what is the rate of consumption of NH3? 4NH3+5O2→NO+4H2O =____moles per liter hour 3)All of the following are true about catalysts, EXCEPT: Select the correct answer below: Catalysts can speed up the rate of a reaction. They cause...
For the following reaction, to get the rate of formation of N2, what must we multiply the rate of consumption of NH3 by? 2NH3---> N2 + 3H2 *Report your answer as a fraction
for the following reaction, to get the rate of formation of H2O - 2x C @ 2 - 2 hours 3/34 QUESTION 7.1 POINT For the following reaction to get the rate of formation of H,O, what must we multiply the rate of formation of Sio, by? 2 Si,H+70,- 4 Si0, +6H,0 Select the correct answer below: 0 0 0 FEEDBACK
The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 7.5 mol of O2 with 1.4 mol of C3H8 will produce ________ mol of CO2. Group of answer choices.
The combustion of propane, C3H8, occurs via the reaction C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) C3H8 (g)= -104.7 CO2(g)= −393.5 H2O(g)= −241.8 Calculate the enthalpy for the combustion of 1 mole of propane.
Consider the following reaction: C3H8+5O2→3CO2+4H2OC3H8+5O2→3CO2+4H2O What is the reducing agent? C3H8C3H8 CC OO O2
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) ΔrH° = -2220 kJ
Propane (C3H8)burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxnΔ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/molkJ/mol.) Express the enthalpy in kilojoules to four significant figures.
How molecules of CO2 (g) are produced when 0.75 moles of propane are burned? Chemical reaction: C3H8 + 5O2 à 3CO2 + 4H2O