The reaction 2NO(g)+2H2(g)N2(g)+2H2O(g) was studied at a certain tempernture wlth the folloyaing rasults: (a) What is the rate law for this reaction? Rate=k[NO(g)]{H2(g)]Rate=k[NO(g)]2[H2(g)]Rate=k[NO(g)][H2(g)]2Rate=k[NO(g)]2[H2(g)]2Rate=k[fO(g)][H2(g)]3Rate=k[NO(g)]4[H2(g)} (a) What is the rete Law for this reaction? Rate=k{NO(g)][H2(g)]Pate=k{NO(g)]2[H2(g)]Rate=k[NO(g)][H2(g)]2Rate=k[NQ(g)]2[H2(g)]2Rate=k[NO(g)][H2(g)]3Rate=k[NO(g)]4[H2(g)] (b) What is the value of the rate constant? (c) What is the reaction race when the cencentration of NO(0) is 0.0951 N and that of H(9) is 0.175M if the ternoeratire is the iame as that used to obtain ene data shown aboive