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Lady_Fox [76]
3 years ago
10

Which of the following would be used to measure the amount of matter in an object?

Chemistry
1 answer:
erik [133]3 years ago
3 0
The answer is Weight
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First, by magnet separate paper clips.
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How many grams of chlorine gas can be produced from the decomposition of 1.46x1023 formula units of AuCl3?
icang [17]

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c

Explanation:

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Through 100 ml of a one-molar sodium hydroxide solution, 896 ml (n.a.) of carbon dioxide was passed gas. Determine the mass solu
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Through 100 ml of a one-molar sodium hydroxide solution, 896 ml (n.a.) of carbon dioxide was passed gas. Determine the mass solution of salt in the resulting solution. Density of a one-molar alkali solution, take equal to 1.04 g / ml.
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3 years ago
To determine the freezing point depression of a LiCl solution, Toni adds 0.317 g of LiCl to the sample test tube along with 20.5
Natali [406]

Answer:

0.365 m

Explanation:

The <em>definition of molality</em> is:

  • molality = moles of solute / kg of solvent

First <u>we calculate the moles of the solute, LiCl</u>. We do so using its <em>molar mass</em>:

  • 0.317 g ÷ 42.394 g/mol = 7.48x10⁻³ mol

Then we calculate the mass of the solvent, water. We do so using its <em>density</em>:

  • 20.5 mL * 0.9982 g/mL = 20.5 g
  • 20.5 g / 1000 = 0.0205 kg

Finally we <u>calculate the molality of the solution</u>:

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4 0
3 years ago
Consider the data [X] [Y] [Z] initial rate M M M M · s −1 Exp 1 0.30 0.20 0.35 0.210 Exp 2 0.60 0.10 0.70 0.420 Exp 3 0.60 0.20
sergij07 [2.7K]

Answer:

Rate = k [X]⁻¹ [Z]²

Explanation:

[X] [Y] [Z] initial rate M M M M · s −1

Exp 1 0.30 0.20 0.35      0.210

Exp 2 0.60 0.10 0.70      0.420

Exp 3 0.60 0.20 0.70     0.420

Exp 4 0.60 0.40 0.35      0.105

In Experiment 2 and 3 where the concentrations of Y and Z were constant, doubling the concentration of Y had no effect on the rate of the reaction. This means, that the rate of the reaction is zero order with respect to Y.

In experiment 3 and 4, dividing the concentration of Z by 2, causes the rate of the reaction to decrease by 4. This means the rate of the reaction is second order with respect to Z.

In experiment 1 and 4, doubling the concentration of X, causes the rate of the reaction to decrease by half. This means that X has an order of -1 with respect to the rate of the reaction.

The rate expression is given as;

Rate = k [X]⁻¹[Y]⁰[Z]²

Rate = k [X]⁻¹ [Z]²

3 0
3 years ago
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