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3 years ago

A reading before and after was taken from a burette, as shown.

Chemistry

1 answer:

mestny [16]3 years ago

7 0

Answer:

Reading on left looks like 1.4

Explanation:

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Determine how many liters 8.65 g of carbon dioxide gas would occupy at the following conditions.

VashaNatasha [74]

1) 6.17 liters

2)2.66 liters

3 0

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:

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

7 0

3 years ago

Name the following alkyne:

xxMikexx [17]

Answer:

7 methyl 3 octyne is the answer option D

7 0

2 years ago

These are three theorized causes of A) glacial melting. B) changing of the climate. C) high and low ocean tides. D) movement of

professor190 [17]

actually its D) movement of tectonic plates

8 0

4 years ago

How many liters of oxygen are required to react with 2.5 grams of magnesium?

emmasim [6.3K]

Answer:

1.16L

Explanation:

First, let us generate the balanced equation for the reaction. This is illustrated below

2Mg + O2 —> 2MgO

Now let us covert 2.5g of Mg given in the question to moles. This is illustrated below:

Molar Mass of Mg = 12g/mol

Mass of Mg = 2.5g

Number of mole of Mg =?

Number of mole = Mass /Molar Mass

Number of mole of Mg = 2.5/24 = 0.104mole

From the equation,

2moles of Mg required 1mole of O2.

Therefore, 0.104mole of Mg will require = 0.104/2 = 0.052mole of O2

Now let us calculate the volume occupy by 0.052mole of O2. This is shown below.

1mole of a gas occupy 22.4L at stp

Therefore, 0.052mole of O2 will occupy = 0.052 x 22.4 = 1.16L

Therefore, 1.16L of O2 is required for the reaction

6 0

3 years ago