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solong [7]
3 years ago
5

What defines endothermic reactions and exothermic reactions? Select all that apply.

Chemistry
2 answers:
Sergio039 [100]3 years ago
7 0

Answer:

The answer to your question is A and B

Explanation:

Chemical reactions can be classified by the energy that they need to proceed or the energy they release.

Endothermic reactions are reactions that require energy to proceed most of the time this energy is in the form of heat.

Exothermic reactions are reactions that release energy to proceed, this energy could be in the form of heat or light.

Sati [7]3 years ago
3 0
The answer should be C
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OCAS GAME
makkiz [27]

ok so this was really confusing, but i think i know the answer. D. ...hairy and ancient hermit crabs and swift, darting minnows and sometimes a

crumbling sand dollar.

7 0
3 years ago
Why is it important for scientists to review and repeat the work of other scientists
guapka [62]

Answer:

Accuracy

Explanation:

It is important for scientists to review the work of other scientists, so they can be sure there are no mistakes or lack of judgement. They repeat to compare results to make hypotheses.

3 0
2 years ago
A student attempts to measure the specific heat capacity of an unknown liquid through repeated trials. She measures its specific
Goryan [66]

Answer:

2.13

Explanation:

4 0
3 years ago
A sample of a compound contains ​0.300 mol​ ​of carbon​ and ​1.20 mol​ ​of hydrogen​. What is the ​empirical formula of the comp
Margarita [4]

Answer:

CH4

Explanation:

The number of moles of carbon and hydrogen has been given as follows:

C = ​0.300 mol​ ​

H = ​1.20 mol

Next, we divide each mole value by the smallest (0.300)

C = 0.300 ÷ 0.300 = 1

H = 1.20 ÷ 0.300 = 4

The empirical ratio of Carbon and Hydrogen is 1:4, hence, the empirical formula is CH4

3 0
3 years ago
Determine the equilibrium constant, Kp, for the following reaction, by using the two reference equations below: 2 NO(g) + O2(g)
klio [65]

Answer:

Kp=3.07x10^6

Explanation:

Hello,

In this case, by knowing the given reference reactions, one could rearrange them as follows:

2 NO(g) \leftrightarrow N_2(g) + O_2(g); Kp_2 = \frac{1}{2.3 x 10^{-19}}=4.35x10^{18}

N_2(g) + 2O_2(g) \leftrightarrow 2NO_2(g);Kp_3=(8.4x10^{-7})^2=7.056x10^{-13}

Subsequently, to obtain the main reaction, we add the aforementioned reference rearranged reactions as shown below (just as reference):

2NO(g)+N_2(g)+2O_2\leftrightarrow 2NO_2(g)+N_2+O_2

Consequently, the equilibrium constant is computed as:

Kp=\frac{[N_2][O_2]}{[NO]^2} * \frac{[NO_2]^2}{[N_2][O_2]^2} =Kp_2*Kp_3=4.35x10^{18}*7.056x10^{-13}=3.07x10^6

Best regards.

8 0
3 years ago
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