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3 years ago

A good experimental design should always:

Chemistry

1 answer:

Alenkinab [10]3 years ago

8 0

Answer:

A good experimental design should always: include more than one independent variable. have predictable outcomes. be repeatable.

Explanation:

Hope this helps :D

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6.How many moles of gas would be in contained in a 11.2 L container that is at a

qaws [65]

0.34 moles of gas would be contained in a 11.2 L container that is at a pressure of 0.75 atm and 300 K.

<h3>HOW TO CALCULATE NUMBER OF MOLES?</h3>

The number of moles of a substance can be calculated using the following expression:

PV = nRT

Where;

p = pressure (atm)
v = volume (L)
n = number of moles
R = gas law constant
T = temperature

0.75 × 11.2 = n × 0.0821 × 300

8.4 = 24.63n

n = 8.4 ÷ 24.63

n = 0.34 moles

Therefore, 0.34 moles of gas would be contained in a 11.2 L container that is at a pressure of 0.75 atm and 300 K.

Learn more about number of moles at: brainly.com/question/1190311

4 0

2 years ago

Be sure to answer all parts. Propane (C3H8) is a minor component of natural gas and is used in domestic cooking and heating. (a)

Leokris [45]

Answer:

For a: The balanced chemical equation is given below.

For b: The mass of carbon dioxide produced will be $1.07\times 10^3g$

Explanation:

For a:

Every balanced chemical equation follows law of conservation of mass.

This law states that mass can neither be created nor can be destroyed but it can only be transformed from one form to another form.

This law also states that the total number of individual atoms on the reactant side must be equal to the total number of individual atoms on the product side.

For the given reaction, the balance chemical equation follows:

$C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)$

All the substances are present in gaseous state.

For b:

By Stoichiometry of the reaction:

1 mole of propane gas produces 3 moles of carbon dioxide gas.

So, 8.11 moles of propane gas will produce = $\frac{3}{1}\times 8.11=24.33mol$ of carbon dioxide gas.

Now, calculating the mass of carbon dioxide using equation:

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

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 24.33 mol

Putting values in above equation, we get:

$24.33mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=1070.52g$

Hence, the amount of $CO_2$ produced in the given reaction and expressed in scientific notation is $1.07\times 10^3g$

3 0

4 years ago

Which process removes carbon dioxide from the atmosphere

Lostsunrise [7]

Answer:

Photosynthesis

Explanation:

6 0

3 years ago

Read 2 more answers

A chemist prepares a solution of vanadium chloride by measuring out of into a volumetric flask and filling to the mark with dist

user100 [1]

The question is incomplete, the complete question is:

A chemist prepares a solution of vanadium (III) chloride (VCl3) by measuring out 0.40g of VCl3 into a 50.mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Cl− anions in the chemist's solution. Be sure your answer is rounded to the correct number of significant digits.

Answer:

0.153M of anions

Explanation:

First we calculate the concentration of the solution. From m/M= CV

m=given mass, M= molar mass, C =concentration of solution, V= volume of solution

Molar mass of compound= 51 + 3(35.5)= 157.5gmol-1

0.4g/157.5gmol-1= C×50/1000

C= 2.54×10-3/0.05= 0.051M

But 1 mole of VCl3 contains 3 moles of anions

Therefore, 0.051M will contain 3×0.051M of anions= 0.153M of anions

4 0

3 years ago

Read 2 more answers

A moose eats a lily pad. The food the moose eats is used to make ATP energy that can be used in cellular processes. The products

AURORKA [14]

Its is B (oxygen) and C (glucose)

6 0

3 years ago