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4 years ago

When taking measurements, you must consider _____.

Chemistry

2 answers:

Karolina [17]4 years ago

7 0

Accuracy, precision, and uncertainty. Hope this helps!!

ss7ja [257]4 years ago

6 0

Hey there!

Your answer is the first option.
When taking measurements, you must consider all:
Accuracy, precision, and uncertainty.

Hope this helps you.
Have a great day!

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The cycle repeats when the carbon stored in the atmosphere as carbon dioxide gas is taken in.

Rzqust [24]

Answer:

Order of the cycle:

Step -1>>>>Step -4 >>>> Step -3 >>>>> step -2.

Explanation:

Step -1:

Carbon dioxide is taken in by plants during photosynthesis.

Step -4;

The animal eats a plant and uses its carbohydrates for energy.

Step - 3

The animal releases the carbon dioxide back into the atmosphere during respiration.

Step -2

The cycle repeats when the carbon stored in the atmosphere as carbon dioxide gas is taken in.

Therefore, order of the cycle is Step -1>>>>Step -4 >>>> Step -3 >>>>> step -2.

5 0

3 years ago

Read 2 more answers

Help me please i need it for homework i cant seen to solve the answer :((

strojnjashka [21]

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7 0

3 years ago

For a reaction to be in equilibrium.... *

IrinaK [193]

Answer: C) the rate of forward reaction is not equal to the rate of backward reaction. This should be the answer.

Explanation:

3 0

3 years ago

17) Chlorine and Fluorine react to form gaseous chlorine trifluoride. You start with 1.75 mole of chlorine and 3.68 moles of flu

Mama L [17]

Answer:

a) $Cl_2 + 3F_2 \rightarrow 2ClF_3$

b) $F_2$ is the limiting reagent

c) Moles of $ClF_3$ produced = 2.45 mol

b) Moles of $Cl_2$ left = 1.75 -1.22 = 0.53

Explanation:

a) Balanced reaction:

$Cl_2 + 3F_2 \rightarrow 2ClF_3$

No. of mole of $Cl_2 = 1.75\ mol$

No. of mole of $F_2 = 3.68\ mol$

$Cl_2 + 3F_2 \rightarrow 2ClF_3$

As, it is clear from the reaction that,

1 mol of $Cl_2$ requires 3 moles of $F_2$

1.75 mol of $Cl_2$ require = 1.75 × 3 = 5.25 mol of $F_2$

As, only 3.68 mol of $F_2$ is present, so $F_2$ is the limiting reagent.

3 moles of $F_2$ form 2 moles of $ClF_3$

3.68 moles of $F_2$ will form = $\frac{2}{3} \times 3.68 = 2.45\ mol\ of\ ClF_3$

$Cl_2$ is present in excess.

3 moles of $F_2$ requires 1 mol of $Cl_2$

3.68 moles of $F_2$ will require = $\frac{1}{3} \times 3.68 = 1.22\ mol\ of\ Cl_2$

$Cl_2$ left = 1.75 -1.22 = 0.53 mol

6 0

4 years ago

Read 2 more answers

Determine the percent yield for the reaction

kkurt [141]

Answer:

The percent yield for Br₂ in the reaction = 96.15%

Explanation:

The balanced stoichiometric equation for the reaction is given as

2 NaBr + 1 Cl₂ → 2 NaCl + 1 Br₂

Percent yield

= 100% × (Actual yield)/(Theoretical yield)

To find the theoretical yield,

5.29 g of NaBr reacts with excess chlorine

gas; this means that NaBr is the limiting reagent because it is used up in the process of the reaction, hence, it determines the amount of products to be found.

So, we convert the 5.29 g of NaBr into number of moles.

Number of moles = (Mass)/(Molar mass)

Molar Mass of NaBr = 102.894 g/mol

Number of moles = (5.29/102.894) = 0.0514121329 = 0.05141 mole

From the stoichiometric balance of the reaction,

2 moles of NaBr give 1 mole of Br₂

0.05141 mole of NaBr will give (0.05141×1/2) mole of Br₂; that is, 0.0257 mole of Br₂

Theoretical yield = Mass of Br₂ expected from the reaction

= (Number of moles) × (Molar mass)

Molar mass of Br₂ = 159.808 g/mol

Theoretical yield of Br₂ = 0.0257 × 159.808 = 4.108 g

Percent yield

= 100% × (Actual yield)/(Theoretical yield)

Actual yield = 3.95 g

Theoretical yield = 4.108 g

Percent yield = 100% × (3.95/4.108) = 96.15%

Hope this Helps!!!

5 0

4 years ago