Hydrogen reacts with nitrogen to form ammonia (NH_3) according to the reaction,
ID: 1065897 • Letter: H
Question
Hydrogen reacts with nitrogen to form ammonia (NH_3) according to the reaction, 3H_2(g) + N_2(g) doubleheadarrow 2 NH_3(g). The value of delta is -92 38 kJ/mol, and that of delta is -198.2 J/mol K. Estimate delta G^+ at 350.00 degree C. + 1.234 times 10^kJ/mol +161.8 kJ/mol -215.9 kJ/mol -23.0 kJ/mol +31.1 kJ/mol Given the following data, dertermine the rate law for the reaction NH_4^-(aq) + NO_2^-(aq) rightarrow N_2(g) + 2H_2 O(c) k[NH_4^+] [NO_2^-] k[NH_4^+]^2 [NO_2^-] k[NH_4^+] [NO_2^-]^1/2 k[NH_4^+]^1/2 [NO_2^-]^2 k[NH_4^+] [NO_2^-]^2 A reaction is first order in A. If the rate constant of the reaction is 3.45 times 10^-3 s^-1, what is the half-life (t_1/2) of the reaction? 4.98 times^-3 s 201 s 3.45 times 10^-3 s 100. S 1.73 times 10^-3 s HI dissociates to form I_2 and H_2; 2 HI(g) rightarrow H_2(g) + I_2(g). If the concentration of HI changes at a rate of -0.45 M/s, what is the rate of appearance of I_2(g)? 0.90M/s 0.45 M/s 0.23 M/s 1.00 M/s 0.13 M/s For the reaction 4 NH_2(g) + 7 O_2(g) rightarrow 4 NO_2 (g) + 6 h_2(g), if H_2 is produced at a rate of 3.5 times 10^_3 M/s. O_2 is consumed at a rate of _______ 2.2 TIMES 10^-2 M/s. 2.1 times 10^-2 M/s. 4.1 times 10^-3 M/s. 3.0 times 10^-3 M/s. 5.8 times 10^-4 M/s. The half-life of radioactive carbon -14 is 5730 years. If the^14C level in a sample of organic matter has been reduced to 0.200% of its original value, approximately how much times has passed? Radioactive decay follows first order kinetics. 1650 years 51, 400 years 29, 900 years 2, 870,000 years 9220 yearsExplanation / Answer
Answer of (24) = (e)
Answer of (25) = (C)
Answer of (26) = (C)
Answer of (27) = (a)
Answer of (28) = (b)
Answer of (29) = (C)
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