CHEMISTRY MIDDLE SCHOOL

Given the following equation: Cu + 2 AgNO3 → Cu(NO3)2 + 2 AgHow many moles of Cu are needed to react with 3.50 moles of AgNO3?
mols

Answers

Answer 1
Answer:

Answer:

1.75 moles of copper are needed to react with 3.50 moles of AgNO₃.

Explanation:

Given data:

Moles of copper needed = ?

Moles of AgNO₃ = 3.50 mol

Solution:

Chemical equation:

Cu + 2AgNO₃  → Cu(NO₃)₂ + 2Ag

Now we will compare the moles of copper and AgNO₃.

                      AgNO₃         :            Cu

                          2               :             1

                        3.50            :             1/2×3.50 = 1.75 mol

So 1.75 moles of copper are needed to react with 3.50 moles of AgNO₃.
Answer 2
Answer:

Final answer:

To find the number of moles of Cu needed to react with 3.50 moles of AgNO3, we can use a proportion from the balanced equation. The number of moles of Cu needed is 1.75 moles.

Explanation:

The balanced equation shows that 1 mole of Cu reacts with 2 moles of AgNO3. Therefore, we can set up a proportion to find the number of moles of Cu needed to react with 3.50 moles of AgNO3 as follows:

Moles of Cu / 1 = 3.50 moles of AgNO3 / 2

By cross-multiplying and solving for the unknown variable, we find that the number of moles of Cu needed is 1.75 moles.

Learn more about stoichiometry here:

brainly.com/question/30218216

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Answers

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Answers

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Answers

9.75 x 10^5

A number in scientific notation has the form a x 10^b where

• a is the coefficient

• b is the exponent

Here are the steps to convert a number greater than 1 to scientific notation.

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Put the decimal point after the first digit and drop the trailing zeroes

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Count the number of digits after the first digit.

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Please tell if this right!if not please answer with correct answers

Answers

Yes I’m. 80% sure that it’s right

Answer:

Yes, you are correct

Explanation:

Nice job :)
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