Calculate the delta for the reaction 4NH_3(x) + 50_2 (x) rightarrow 4NO(x) + 6H_

Question

Calculate the delta for the reaction 4NH_3(x) + 50_2 (x) rightarrow 4NO(x) + 6H_2O(x) -908.4 KJ -106.l kJ 106.l kJ 908.4 kJ What is the atomic molar mass of X in K_2X_2O_3, if the formula molar mass of this compound is 294 g mol^1g 26.0 g mol^1 52.0 g mol^1 104 g mol^1 147 g mol^1 Element X, consisting of two isotopes, has an average atomic mass of 15.91 u. if the atomic mass of the first isotope is 15.88 u and has a naturally occurring abundance of 92.10 percent, what is the atomic mass of the second isotope? 14.65 u 15.90 u 15.91 u 16.26 u Which isotopic variation of water contains the highest percentage of hydrogen by weight?^2H -^17O -^2H^1H -^16O -^2H^1H -^19O -^3H^1H -^16O -^3H What is the molecular formula of a compound that has a molar mass of 80.5 g mol^-1 if it has an empirical formula BNH_2? BNH_2 B_2N_2H_4 B_3N_3H_6 B_4N_2H_9 A substance composed only of nitrogen and oxygen contains 63.2 percent oxygen by weight. What is its empirical formula? N_2O NO_2 N_2O_3 N_2O_5 A compound has the general formula X_2O_3. Laboratory analysis shows that a 10.0 g sample of the compound contains 5.29 g of the element X. What is the element? N P As Al

Explanation / Answer

Question 16

Delta H = 4 (89.8) + 6 (-242) - 4(-46.1)

Delta H = -908.4 kj

Hence answer is A

Question 17

K2X2O7 = 294

2 (39.09) + 2 x + 7 (16) = 294

x = 52

Answer is B

Question 18

15.88 (0.9210) + x ( 0.079) = 15.91

x = 16.26 u

Hence answer is D

Question 19

1H- 19O-3H - Answer C (All having higher mass)

Question 20

B3N3H6 Option C (Molar mass of B3N3H6 is 80.5007 g/mol)

Question 21

Answer is N2O Option A

Question 22

Al2O3 Option D

Symbol Element Atomic weight Atoms Mass percent N Nitrogen 14.0067 2 36.8541 % O Oxygen 15.9994 3 63.1459 %

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