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3 years ago

It is possible for an object’s weight to change while it’s mass remains constant?Explain.

Chemistry

1 answer:

NeX [460]3 years ago

6 0

Answer:

Yes

Explanation:

An object's weight can change, depending on its location, relative to the object of discussion. For example, we don't notice the change, but the farther away we are from Earth's core, the less we weigh. This means one would weigh more in a valley than they would on a mountain. The formula for gravity is F=G((msub1)(msub2)/r^2), where F is the force of attraction, G is the universal gravitational constant, msub1 is the mass of the first object, msub2 is the mass of the second object, and r is the distance between the two objects.

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what volume, in liters, will 6.32 × 10^2 of air occupy if the density of air is 1.29 g/L? Express your answer in scientific nota

xz_007 [3.2K]

4.90× 10^2 L

I am guessing that the mass of the air is 6.32 × 10^2 <em>g</em>. Then,

Volume = 6.32 × 10^2 g × (1 L/1.29 g) = 4.90× 10^2 L

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3 years ago

Read 2 more answers

In this reaction: Mg (s) + I₂ (s) → MgI₂ (s) If 2.68 moles of Mg react with 3.56 moles of I₂, and 1.76 moles of MgI₂ form, what

melomori [17]

Answer:

$Y=65.7\%$

Explanation:

Hello,

In this case, for the given chemical reaction, we first identify the limiting reactant by noticing that due to the 1:1 mole ratio for magnesium to iodine the reacting moles must the same, nevertheless, there are only 2.68 moles of magnesium versus 3.56 moles of iodine, for that reason, magnesium is the limiting reactant, so the theoretical turns out:

$n_{MgI_2}^{theoretical}=2.68molMg*\frac{1molMgI_2}{1molMg} =2.68molMgI_2$

Thus, we compute the percent yield as:

$Y=\frac{n_{MgI_2}^{real}}{n_{MgI_2}^{theoretical}} *100\%=\frac{1.76mol}{2.68mol} *100\%\\\\Y=65.7\%$

Best regards.

8 0

3 years ago

What is the percent yield of LiCl if I produced 30.85g LiCl and my theoretical yield was calculated to be 35.40g LiCl?

marissa [1.9K]

Answer:

87.15%

Explanation:

To find percent yield, we can use this simple equation

$\frac{Actual}{Theoretical} *100$

Where "Actual" is the amount in grams actually collected from the reaction, and "Theoretical" is, well, the theoretical amount that should have been produced.

They give us these values, so to find the percent yield, just plug the numbers in.

$\frac{30.85}{35.40} *100\\\\ =87.15$

So, the percent yield is 87.15%

An easy trick to remember how to do this is just to divide the smaller number by the bigger number and move the decimal back two places. If you have a percent yield greater than 100%, something is wrong in the reaction.

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3 years ago

Why are these graphs misleading

ch4aika [34]

Although there isn’t a picture a graph can be misleading when it doesn’t start at zero, it doesn’t give accurate information, it skips too many numbers, the vertical scale is too big or too small. Hope this helps

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3 years ago

The balanced equation shows how sodium chloride reacts with silver nitrate to form sodium nitrate and silver chloride. NaCl + Ag

Verdich [7]

<span>NaCl First calculate the molar mass of NaCl and AgNO3 by looking up the atomic weights of each element used in either compound Sodium = 22.989769 Chlorine = 35.453 Silver = 107.8682 Nitrogen = 14.0067 Oxygen = 15.999 Now multiply the atomic weight of each element by the number of times that element is in each compound and sum the results For NaCl 22.989769 + 35.453 = 58.44277 For AgNO3 107.8682 + 14.0067 + 3 * 15.999 = 169.8719 Now calculate how many moles of each substance by dividing the total mass by the molar mass For NaCl 4.00 g / 58.44277 g/mol = 0.068443 mol For AgNO3 10.00 g / 169.8719 g/mol = 0.058868 Looking at the balanced equation for the reaction, there is a 1 to 1 ratio in molecules for the reaction. Since there is a smaller number of moles of AgNO3 than there is of NaCl, that means that there will be some NaCl unreacted, so the excess reactant is NaCl</span>

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3 years ago