3 years ago

HURRY!!!!!!!!!!!!!!!!

Chemistry

2 answers:

steposvetlana [31]3 years ago

8 0

Answer:A. The deodorant evaporates as it absorbs thermal energy from James’s skin.

Explanation:

Rasek [7]3 years ago

4 0

I think the answer would be A

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Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 2 al(s) + 6 hcl(aq) → 2 alcl3(aq) + 3 h2(g

MariettaO [177]

Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 2 al(s) + 6 hcl(aq) → 2 alcl3(aq) + 3 h2(g) what mass of h2(g) is produced from the reaction of 1.35 g al(s) with excess hydrochloric acid?

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4 years ago

Calculate the percent yield of a reaction where a student collected 16.8 grams of product and was expecting to collect 49.7 gram

masya89 [10]

Answer:

$\boxed{\text{33.8 \%}}$

Explanation:

$\text{\% yield} = \dfrac{\text{actual yield}}{\text {theoretical yield}} \times\text{100 \%}$

Data:

Actual yield = 16.8 g

Theoretical yield = 49.7 g

Calculation:

$\text{\% yield} = \dfrac{\text{16.8 g}}{\text {49.7 g}} \times\text{100 \%} = \boxed{\textbf{33.8 \%}}$

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3 years ago

As the temperature increases, the molecular motion of the molecules decreases and it

inn [45]

Answer:

true

Explanation:

i'm not so sure

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3 years ago

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The first season of Stranger Things consists of eight episodes. Each episode is approximately

OLga [1]

Answer:

You will be watching for 6 hours

Explanation:

We will have 45 x 8 which will give us 360 then we divide it by 60 which will give us 6.

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3 years ago

The combustion of ethane (C2H6)(C2H6) produces carbon dioxide and steam. 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(g) 2C2H6(g)+7O2(g)⟶4CO2(g)

Vera_Pavlovna [14]

Answer:

11.9 moles of carbon-dioxide will produced.

Explanation:

Given moles of ethane = 5.95 mol

$2C_2H_6(g)+7O_2(g)\rightarrow 4CO_2(g)+6H_2O(g)$

According to reaction 2 moles of ethane produces 4 moles of carbon-dioxide.

Then, 5.95 moles of ethane will produce:

$\frac{4}{2}\times 5.95 mol=11.9 mol$ of carbon-dioxide

11.9 moles of carbon-dioxide will produced.

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3 years ago