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Gre4nikov [31]
3 years ago
10

Determine whether the variable is qualitative or quantitative. grams of carbohydrates in a donut. grams of carbohydrates in a do

nut
Chemistry
1 answer:
Sophie [7]3 years ago
4 0
You would know that the variable is quantitative if it shows any number to express the quantity. For example, quantitative variables are 50°C, 5 atm, 2 moles, 100 L and so on. A variable is qualitative if it expresses a relative quantity but not expressing a number. Examples would be: few, too hot, several, or even describing the characteristics of a variable. Hence, when the variable is in grams, then that would be quantitative.
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Recall the formula of glucose is c 6 h 12 o 6 . how many carbon, oxygen, and hydrogen atoms will you need for three glucose mole
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3 C6H12O6, 
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7 0
3 years ago
Convert 44.8 liters of CO2 into particles of CO2​
jonny [76]

Answer:

1.2044 x 10^24 particles

Explanation:

Assuming this is<u> STP</u>....then this is 2 moles    ( each mole = 22.4 L/mole)

  2 moles = 2 * 6.022 x 10^23  = 1.2044 x 10^24

               

5 0
2 years ago
A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL soluti
Kaylis [27]

<u>Answer:</u> The value of K_a for the given acid is 3.58\times 10^{-4}

<u>Explanation:</u>

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)}}

Initial mass of weak monoprotic acid = 1.00 g

Molar mass of weak monoprotic acid = 180 g/mol

Volume of solution = 300 mL

Putting values in above equation, we get:

\text{Molarity of weak monoprotic acid}=\frac{1.00\times 1000}{180\times 300}\\\\\text{Molarity of weak monoprotic acid}=0.0185M

To calculate the hydrogen ion concentration for given pH of the solution, we use the equation:

pH=-\log[H^+]

We are given:

pH = 2.62

Putting values in above equation, we get:

2.62=-\log[H^+]

[H^+]=10^{-2.62}=2.40\times 10^{-3}M=0.0024M

The chemical equation for the dissociation of weak monoprotic acid (HA) follows:

                            HA\rightleftharpoons H^++A^-

<u>Initial:</u>              0.0185

<u>At eqllm:</u>        0.0185-x     x     x

Evaluating the value of 'x'

\Rightarrow x=0.0024

So, equilibrium concentration of HA = (0.0185 - 0.0024) = 0.0161 M

Equilibrium concentration of A^- = x = 0.0024 M

The expression of K_a for above equation follows:

K_a=\frac{[H^+][A^-]}{[HA]}

Putting values in above equation, we get:

K_a=\frac{(0.0024)\times (0.0024)}{0.0161}=3.58\times 10^{-4}

Hence, the value of K_a for the given acid is 3.58\times 10^{-4}

5 0
4 years ago
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