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3 years ago

For the following reaction, predict whether the equilibrium lies predominantly to the left or to the right. Explain.

Chemistry

1 answer:

Likurg_2 [28]3 years ago

6 0

Answer:

Lies predominantly to the left.

Explanation:

In the reaction:

NH4⁺(aq) + Br-(aq) ⇄ NH3(aq) + HBr(aq)

Conjugate acid + Ion ⇄ weak base + strong acid

HBr is a strong acid whereas NH3/NH4⁺ are the weak base and its conjugate base. A strong acid as HBr dissociates completely in solution as H⁺ and Br⁻. That means in solution you will never have HBr without dissociation doing the reaction:

<h3>lies predominantly to the left.</h3>

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A sample of gas in a cylinder as in the example in Part A has an initial volume of 48.0 L , and you have determined that it cont

masya89 [10]

Answer:

0.45 moles

Explanation:

The computation of the number of moles left in the cylinder is shown below:

As we know that

$\frac{n1}{V1} = \frac{n2}{V2}$

we can say that

$n2 = n1 \times \frac{V2}{V1}$

where,

n1 = 1.80 moles of gas

V2 = 12.0 L

And, the V1 = 48.0 L

Now placing these values to the above formula

So, the moles of gas in n2 left is

$= 1.80 \times \frac{12.0\ L}{48.0\ L}$

= 0.45 moles

We simply applied the above formulas so that the n2 moles of gas could arrive

5 0

3 years ago

What is a common use of bases?

Fittoniya [83]

A common use of bases is to reduce indigestion. Hence, option D is correct.

A base is a substance that can neutralize the acid by reacting with hydrogen ions.

Bases are substances whose solutions have a pH value of more than 7. Bases are bitter in taste.

Whereas acids are the substances whose solutions have a pH value of less than 7. Acids are sour in taste.

When an excess of acid is formed in the human stomach then an antacid tablet which is basically a base is consumed that helps in reducing indigestion.

Therefore, we can conclude that the common use of bases is to reduce indigestion.

Learn more about the base here:

brainly.com/question/1432645

#SPJ1

3 0

2 years ago

How many liters or oxygen gas is required to react with 50.0g of aluminum at STP?

suter [353]

Answer:

aluminum oxide will be produced from the complete reaction of 1.87L of oxygen gas at 793.0mmHg and 28.0 Celsius. answer: 5.36g

Explanation:

7 0

3 years ago

What's the constant presuure of gas?

pickupchik [31]

Answer:

Constant pressure of gas must have a constant volume and a constant number of moles of gas. It's equation is the ideal gas law: pV=nRT

Explanation:

The gas state is the most excited state. It doesn't have a definite volume or shape which is why it can be compressed. Gas pressure is basically the result of all the gas particles moving around and colliding against each other and their container. The rate this happens at as well as its force determines the pressure. Since there are many, many of these gas particles in all quantities of gas, the fluctuation of this rate as well as its intesity is nearly constant.

5 0

3 years ago

A chemist requires 5.00 liters of 0.420 M H2SO4 solution. How many grams of H2SO4 should the chemist dissolve in water? 129 gram

natali 33 [55]

Answer:

Approximately 206 grams.

Explanation:

How many moles of sulfuric acid $\mathrm{H_2SO_4}$ are there in this solution?

$\text{Number of moles of solute} = \text{Concentration} \times \text{Volume}$ .

The unit for concentration " $\mathrm{M}$ " is equivalent to mole per liter. In other words, $\rm 1\;M = 1\; mol\cdot L^{-1}$ . For this solution, the concentration of $\mathrm{H_2SO_4}$ is $\rm 0.420\;M = 0.420\; mol\cdot L^{-1}$ .

$\begin{aligned}n(\mathrm{H_2SO_4}) &= c(\mathrm{H_2SO_4}) \cdot V\\&= \rm 0.420\;mol\cdot L^{-1}\times 5.00\; L \\&= \rm 2.10\; mol\end{aligned}$ .

What's the mass of that $\rm 2.10\; mol$ of $\mathrm{H_2SO_4}$ ?

Start by finding the molar mass $M$ of $\mathrm{H_2SO_4}$ .

Relative atomic mass data from a modern periodic table:

H: 1.008;
S: 32.06;
O: 15.999.

$\displaystyle M(\mathrm{H_2SO_4}) = 2\times \underbrace{1.008}_{\mathrm{H}} + 1\times \underbrace{32.06}_{\mathrm{S}} + 4\times \underbrace{15.999}_{\mathrm{O}} = \rm 98.072\;g\cdot mol^{-1}$ .

$\text{Mass} = \text{Quantity in moles} \times \text{Molar Mass}$ .

$m = n \cdot M = \rm 2.10\; mol \times 98.072\;g\cdot mol^{-1} \approx 206\; g$ .

In other words, the chemist shall need approximately 206 grams of $\mathrm{H_2SO_4}$ to make this solution. As a side note, keep in mind that the 206 grams of $\mathrm{H_2SO_4}$ also take up considerable amount of space. Therefore it will take less than 5.00 L of water to make the 5.00 L solution.

6 0

3 years ago