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0.866 J/g·0C
2.60 J/g·0C
0.650 J/g·0C
1.15 J/g·0C
2.83 × 105 J/g·0C
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32.00C
46.20C
47.20C
57.20C
65.0C
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0.055 J/g· 0C
0.29 J/g · 0C
0.69 J/g · 0C
0.18 J/g · 0C
2.6 J/g · 0C
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55.37 C
58.60 C
59.40 C
60.80 C
64.19 C
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–116 J/g
–934 J/g
–1.03 × 103 J/g
–2.19 × 103 J/g
–1.03 × 104 J/g
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0.00 0C
2.24 0C
5.22 0C
25.0 0C
47.8 0C
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Hess' law states that ΔH for an overall reaction is the sum of the ΔH values for the individual equations.
The molar enthalpy of formation of a compound is equal to the enthalpy change when one mole of the compound is formed from elements.
A reaction with a negative enthalpy is exothermic.
The enthalpy of formation of an element in its most stable state is equal to zero.
The sum of the enthalpies of formation of the products in a chemical reaction is defined as the enthalpy of reaction.
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+30.24 kJ
–206.9 kJ
–298.6 kJ
–1398.8 kJ
–1663.6 kJ
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–10.3 kJ
–20.7 kJ
–29.8 kJ
–43.7 kJ
–65.6 kJ
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A: +
B: 3
C: 1/2
D: -1/3
E: -
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3.44 × 10-4 mol/L·s
2.07 × 102 mol/L·s
1.24 mol/L·s
74.4 mol/L·s
4.64 × 103 mol/L·s
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–0.360 mol/L·s
–0.090 mol/L·s
0.090 mol/L·s
0.180 mol/L·s
0.360 mol/L·s
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0
1
2
5
7
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Rate = 0.515[A] x [B]
Rate = 0.515[A]^2 x [B]
Rate = 0.721[A]^2 x [B]
Rate = 0.721[A] x [B]^2
Rate = 0.721[A]^2 x [B]^2
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Rate = 8.71 × 104[A]2 × [B] × [C]
Rate = 5.23 × 104[A] × [B]2 × [C]
Rate = 2.90 × 103[A]2 × [B] × [C]2
Rate = 8.71 × 104[A] × [B] × [C]2
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8.72 × 105 M
0.0645 M
0.115 M
0.0785 M
0.643 M
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0.00114 s
1.07 s
2.64 s
38.4 s
874 s
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0.0050 M
0.051 M
0.51 M
0.11 M
2.0 × 102 M
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0.0341 M
0.183 M
1.34 M
2.68 M
29.3 M
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2.0 × 10^1 s
7.8 × 10^1 s
1.8 × 10^2 s
1.9 × 10^2 s
2.2 × 10^2 s
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18 s
24 s
36 s
48 s
51 s
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1 only
2 only
3 only
2 and 3
1, 2, and 3
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0.30
0.55
0.85
1.8
3.3
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0.00153
0.00308
0.00611
0.00730
0.02471
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0.22 atm
0.31 atm
0.47 atm
0.47 atm
0.65 atm
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1 only
2 only
3 only
1 and 2
1 and 3
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7.5 × 10^-16
1.3 × 10^-8
1.4 × 10^-38
1.3 × 10^-15
1.0 * 10^-23
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