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3 years ago

ANSWER QUICKLY PLEASE

Chemistry

2 answers:

bixtya [17]3 years ago

5 0

Answer: A

Explanation:

It's separates naturally due to the consistency of each ingredient in the milk making some of it sink down and you don't want a bad milk

Leni [432]3 years ago

4 0

Answer: option A. naturally

Explanation: since the label suggests shaking the mixture well, it therefore means that the mixture will separate naturally.

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A ____usually requires calculations that are too complicated to do by hand.

liraira [26]

Answer:

computer model

Explanation:

Computer models are cheaper to set up than alternative methods that could be used to predict what will happen in a system, ex. building a prototype. Other benefits include being able to: make alterations and quickly see the outcomes.

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3 years ago

What is the total number of grams of mg consumed when 0.50 mole of h2 is produced

rosijanka [135]

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1 year ago

What is the concentration of a solution that has 15.0 g NaCl dissolved to a total of 750 ml?

Oksana_A [137]

Answer: The concentration of solution is 0.342 M

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

We are given:

Mass of solute (Sodium chloride) = 15 g

Molar mass of sodium chloride = 58.5 g/mol

Volume of solution = 750 mL

Putting values in above equation, we get:

$\text{Molarity of solution}=\frac{15g\times 1000}{58.5g/mol\times 750mL}\\\\\text{Molarity of solution}=0.342M$

Hence, the concentration of solution is 0.342 M

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2 years ago

PLEASE HELP!!! How many grams are in 10.11 moles of sucrose?

Sloan [31]

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2 years ago

Ammonia (NH3) reacts with oxygen to form nitric oxide (NO) and water vapor: 4NH3 + 502 4NO + 6H2O b) When 20.0 g NH3 and 50.0 g

Solnce55 [7]

Answer: a) . Ammonia is the limiting reagent

b. Oxygen is left over and 0.1375 g of oxygen is left over.

c. The theoretical yield of $NO$ is 35.29 g.

d. The theoretical yield of $H_2O$ is 31.74 g.

Explanation:

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

For $NH_3$

Given mass of ammonia = 20.0 g

Molar mass of ammonia = 17.031 g/mol

Putting values in equation 1, we get:

$\text{Moles of ammonia}=\frac{20.0g}{17.031g/mol}=1.17mol$

For $O_2$

Given mass of oxygen gas = 50.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{50.0g}{32g/mol}=1.6mol$

The chemical equation for the reaction is

$4NH_3+5O_2\rightarrow 4NO+6H_2O$

By Stoichiometry of the reaction:

4 moles of ammonia reacts with = 5 moles of oxygen

So 1.17 moles of ammonia will react with = $\frac{5}{4}\times 1.17=1.4625mol$ of oxygen

As, given amount of oxygen is more than the required amount. So, it is considered as an excess reagent and (1.6-1.4625)= 0.1375 g of oxygen is left unreacted.

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

1. By Stoichiometry of the reaction:

4 moles of ammonia produces = 4 moles of $NO$

1.17 moles of ammonia will produce = $\frac{4}{4}\times 1.17=1.17moles$ of $NO$