jhope

This page lists questions and answers that were posted by visitors named jhope.

Questions

The following questions were asked by visitors named jhope.

If it requires 115 J of heat to increase the temperature of 2.17 moles of a solid metal from 24.37 °C to 26.32 °C at constant pressure, then what is the identity of the metal?

Consider the process below. The normal boiling point of CH3CH2CH(OH)CH3 is 99 °C. CH3CH2CH(OH)CH3(g, 128 °C, 1 atm) ⟶ CH3CH2CH(OH)CH3(l, 88 °C, 1 atm) You may assume that the temperature of the surroundings is constant and also equal to 88 °C. Which of th...

For the reaction below at 298.15 K, the standard enthalpy of reaction is ΔrH° = 41.6 kJ mol−1 and the thermodynamic equilibrium constant is K = 1.50×10−6. 2 NO(g) + I2(s) ⇌ 2 NOI(g) What is ΔrS° for this reaction? Do I need to take the K value into consid...

A(aq) + 2 B(aq) ‌⟶ 4 C(aq) + 4 D(aq) What is the rate of production of C, in mol L−1 s−1, if the rate of production of D is 0.310 mol L−1 s−1 ?

The reaction below is second-order in NO and first order in O2. 2 NO(g) + O2(g) ⟶ 2 NO2(g) When 5.00 mol of NO and 2.00 mol O2 were reacted in a 1.00 L flask, the initial rate was 3.9×10−3 M s−1. What is the rate when 50% of the oxygen has reacted? no ide...

The decomposition reaction, X → products, has rate constant k = 0.00707 mol L−1 s−1 at a particular temperature. How long will it take for the decomposition to be 90% complete, if the initial concentration of X is 1.65 mol L−1 ?

Consider the following reaction. CaC2(s) + 2 H2O(l) ⇌ Ca(OH)2(aq) + C2H2(g) Which of the following represents the thermodynamic equilibrium constant, K ? K=[H2O]2[CaC2]PC2H2[Ca(OH)2] K=PC2H2[Ca(OH)2][CaC2] K=[C2H2][Ca(OH)2][H2O]2[CaC2] K=PC2H2[Ca(OH)2] K=...

Consider the following equilibrium. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Determine Kc if 1.00 mol of NOCl(g) is initially placed in an empty 1.00 L flask, and 90% of the NOCl is consumed when the reaction reaches equilibrium.

For the following reaction, Kc = 2.7×108 at 300 K. 3 H2(g) + N2(g) ⇌ 2 NH3(g) In an experiment carried out at 300 K, the initial concentrations of H2(g) and N2(g) are each equal to 2.0 mol L−1 . Which of the following statements about the equilibrium conc...

(1) MgCO3(s) ⟶ MgO(s) + CO2(g) ΔrH = 118.1 kJ mol−1 (2) Mg(s) + 12O2(g) ⟶ MgO(s) ΔfH =−601.7 kJ mol−1 What is the enthalpy change, ΔrH for the following reaction? 2 MgCO3 ⟶ 2 Mg(s) + 2 CO2(g) + O2(g)

Answers

The following answers were posted by visitors named jhope.

dose anyone know the awnsers to Lesson 19: Unit Test Language Arts 6 A Unit 2: Characters and Conflict?

a and c B D THESE ARE THE RIGHT AWNERES ENJOY ._.

thats what i thought, thanks!

hmm never learned those, but thanks

dGo = -RT*lnK for this would it be -8.135(298)ln(298)?

still confused..

what would k be then?

yeah, not sure how to solve it. ive subtracted the temp, but what do i do with the mols and J?

i think its: The entropy of the system increases: ΔS > 0. The entropy of the universe increases: ΔSuniv > 0. Work is done by the system on the surroundings. The process is thermodynamically irreversible. pls confirm

so it would be k=0.0088?

so, 118x-601 + 2x601?

no i dont think thats right

oh i see, is it K=PC2H2[Ca(OH)2]

i mean K=[C2H2][Ca(OH)2]

so it will be: Kc = [Cl2][NO]^2 / [NOCl]^2 =0.9x0.9^2 / 0.9-1?

what do you mean?