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3 years ago

What are the standard ways to make a solution of known concentration? (select all that apply.)?

Chemistry

1 answer:

MatroZZZ [7]3 years ago

8 0

1- Molar solutions: based on number of moles of chemical in 1 litre of solution

2- Weight % solution: the weight of chemical divided by the total weight of the solution (chemical + water) and multiplied by 100.

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3 years ago

Read the given chemical reaction.

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3 years ago

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In a process for producing acetic acid, oxygen gas is bubbled into acetaldehyde, CH3CHO, containing manganese(II) acetate (catal

grigory [225]

Answer: The mass of acetic acid that can be produced is 30.24 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For acetaldehyde:

Given mass of acetaldehyde = 22.2 g

Molar mass of acetaldehyde = 44 g/mol

Putting values in equation 1, we get:

$\text{Moles of acetaldehyde}=\frac{22.2g}{44g/mol}=0.504mol$

For oxygen gas:

Given mass of oxygen gas = 12.6 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{12.6g}{32g/mol}=0.394mol$

The given chemical equation follows:

$2CH_3CHO(l)+O_2(g)\rightarrow 2CH_3COOH(l)$

By Stoichiometry of the reaction:

2 moles of acetaldehyde reacts with 1 mole of oxygen gas

So, 0.504 moles of acetaldehyde will react with = $\frac{1}{2}\times 0.504=0.252mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, acetaldehyde is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of acetaldehyde produces 2 moles of acetic acid

So, 0.504 moles of acetaldehyde will produce = $\frac{2}{2}\times 0.504=0.504moles$ of acetic acid

Now, calculating the mass of acetic acid from equation 1, we get:

Molar mass of acetic acid = 60 g/mol

Moles of acetic acid = 0.504 moles

Putting values in equation 1, we get:

$0.504mol=\frac{\text{Mass of acetic acid}}{60g/mol}\\\\\text{Mass of acetic acid}=(0.504mol\times 60g/mol)=30.24g$

Hence, the mass of acetic acid that can be produced is 30.24 grams

8 0

3 years ago

What is the mass of 1.25 L of ammonia gas at STP

Alex73 [517]

Answer:

mass 1.25 Liters NH₃(gas) = 0.949 grams (3 sig-figs)

Explanation:

At STP (Standard Temperature-Pressure conditions => 0°C(=273K) and 1atm pressure, 1 mole any gas will occupy 22.4 Liters.

So, given 1.25 Liters ammonia gas at STP, convert to moles then multiply by formula wt. (17g/mole gives mass of NH₃.

moles NH₃(gas) = 1.25L NH₃(gas)/22.4L NH₄(gas)· NH₃(gas)mole⁻¹ = 0.0558 mole NH₃(gas).

Converting to grams NH₃(gas) = 0.0558 mole NH₃(gas) x 17 g·mol⁻¹ = 0.949 grams NH₃(gas).

7 0

3 years ago

4. Identify the different parts to this word problem. A bowling ball of 35.2kg, generates 218 kg.m/s units of momentum. What is

Dafna1 [17]

Given:

Mass of the ball = 35.2 kg

Momentum = 218 kg m/s

To determine:

The velocity of the ball

Explanation:

Momentum (p) of an object is the product of its mass (m) and velocity (v)

p = m*v

v = p/m = 218 kg.ms-1/35.2 kg = 6.19 m/s

Ans: The velocity of the ball is 6.19 m/s

3 0

3 years ago