Question 2 of 2SubmitConsider the following reaction:4NH3(g) + 502(g) → 4NO(g) +6H;0(g)If 1.30 L of NH3 reacts with O, at1.50 atm and 32.0°C, what volumeof oxygen is needed for thereaction?L1246.C78+/-x 10 03.LO

Chemical reactions are those reactions which undergo any chemical change. Chemical reaction is represented in chemical equation. Reactants are on the left side of the equation and products are on the right side of the equation.Pressure of the gas, P = 1.50 atm Volume of the ammonia gas, V = 1.30 L Gas constant, R = 0.0821 atm L mol-1K-1 Temperature, T = 305 K The balanced reaction is given as follows: 4NH3g+5O2g→4NOg+6H2Og Using ideal gas equation: PV=nRT Pressure of the gas is P. Volume of the gas is V. No. of moles are n. Gas constant is R. Temperature is T. Substitute these values in the above equation, PV=nRTn=PVRT=1.30×1.500.0821×305=0.078 moles 4 moles of NH3 need = 5 moles of O2 1 mole of NH3 need = 54 moles of O20.078 moles of NH3 need =54×0.078 moles of O2 =0.097 moles PV=nRTV=nRTP=0.097×0.0821×3051.50=1.625 L

Answered: Consider the following reaction:…

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Consider the following reaction: 4NH3(g) + 502(g) → 4NO(g) + 6H;0(g) If 1.30 L of NH3 reacts with O2 at 1.50 atm and 32.0°C, what volume of oxygen is needed for the reaction?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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