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1 year ago

27. What pattern in the behavior of gases is shown from Step I through Step 3 of the figure?

Chemistry

1 answer:

sleet_krkn [62]1 year ago

7 0

Answer:

Boyle's law

Explanation:

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Flammability is an example of what?

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Combustible more specific answer chemical reaction

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4 years ago

How are sunspots correlated with the sun's activity?

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If sunspots are active, more solar flares will result creating an increase in geomagnetic storm activity for Earth.

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3 years ago

The surface tension of which of the following liquid is maximum?

Elden [556K]

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3 years ago

Put the rules in order, first rule up top.

ValentinkaMS [17]

Answer:

Write down the elements
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3 years ago

Consider the following intermediate chemical equations.(IMAGE) -205.7 kJ -113.4 kJ -14.3 kJ 78.0 kJ

andrey2020 [161]

Answer:

Approximately $-205.7\; \rm kJ$ .

Explanation:

This question can be solved using Hess's Law.

Start by considering: how can the first three reactions (with known $\Delta H$ values) be combined to produce the reaction $\rm CH_4\; (g) + 4\; \rm Cl_2\; (g) \to CCl_4\; (g) + 4\; HCl\; (g)$ ?

Here's one possible combination:

Include the first reaction once, without inverting.
Invert the second reaction and include it once.
Include the third reaction after multiplying all its coefficients by two.

In other words, if $(1)$ , $(2)$ , and $(3)$ denote the three reactions with know $\Delta H$ values, respectively, then $1 \times (1) - 1 \times (2) + 2\times (3)$ will give the required reaction $\rm CH_4\; (g) + 4\; \rm Cl_2\; (g) \to CCl_4\; (g) + 4\; HCl\; (g)$ .

By Hess's Law, the $\Delta H$ value of the reaction $\rm CH_4\; (g) + 4\; \rm Cl_2\; (g) \to CCl_4\; (g) + 4\; HCl\; (g)$ will thus be:

$\begin{aligned}&1 \times \Delta H_1 - 1\times \Delta H_2 + 2\times \Delta H_3\\ &= 1 \times 74.6\; \rm kJ - 1 \times 95.7\; \rm kJ +2 \times (-92.3\; \rm kJ) \\ &= -205.7\; \rm kJ\end{aligned}$ .

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3 years ago