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yulyashka [42]
3 years ago
10

What is the slope of the line?

Chemistry
1 answer:
pychu [463]3 years ago
3 0

Answer:

The slope of the line is -\frac{10}{7}.

Explanation:

The slope of the line (m) is the change in dependent variable (y) divided by the change in independent variable (x):

m = \frac{y_{f}-y_{o}}{x_{f}-x_{o}} (1)

If we know that (x_{o}, y_{o}) = (0, 2) and (x_{f}, y_{f}) = (1.4, 0), then the slope of the line is:

m = \frac{0-2}{1.4-0}

m = -\frac{10}{7}

The slope of the line is -\frac{10}{7}.

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What is the approximate percent by mass of potassium in KHCO3?
lozanna [386]

Answer:

The mass percent of potassium is 39%

Option C is correct

Explanation:

Step 1: Data given

Atomic mass of K = 39.10 g/mol

Atomic mass of H = 1.01 g/mol

Atomic mass of C = 12.01 g/mol

Atomic mass of O = 16.0 g/mol

Step 2: Calculate molar mass of KHCO3

Molar mass KHCO3 = 39.10 + 12.01 + 1.01 + 3*16.0

Molar mass KHCO3 = 100.12 g/mol

Step 3: Calculate mass percent of potassium (K)

%K = (atomic mass of K / molar mass of KHCO3) * 100%

%K = (39.10 / 100.12) * 100%

%K = 39.05 %

The mass percent of potassium is 39%

Option C is correct

8 0
3 years ago
1 mole solution of NaCl contains
Mamont248 [21]

Answer:

If you dissolve 58.44g of NaCl in a final volume of 1 liter, you have made a 1M NaCl solution, a 1 molar solution.

Explanation:

7 0
4 years ago
In experiment 1, how many moles of benzoic acid are present? how many moles of sodium bicarbonate are contained in 1 ml of a 10%
nexus9112 [7]

First, let us calculate the moles of solute or sodium bicarbonate is in the 1 ml solution.

<span>moles  = 1 mL * (1 g / 9 mL) = 0.11 moles</span>

 

The molar mass of sodium bicarbonate is 84 g/mol, therefore the mass is:

mass = 0.11 moles * 84 g/mol

<span>mass = 9.33 g</span>

6 0
3 years ago
What are the values of the missing force?
sweet [91]
B=150N A=12N………………………
7 0
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Unbalanced forces can cause an object change its motion in three ways. What are they?
fenix001 [56]
Accelerate, decelerate, and changing directions.
4 0
4 years ago
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