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3 years ago

Photosynthesis is an example of a

Chemistry

1 answer:

Whitepunk [10]3 years ago

7 0

Answer:

An example of photosynthesis is how plants convert sugar and energy from water, air and sunlight into energy to grow.

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Which statements correctly describe thermal energy in a block of ice, a glass of liquid water, and a container of steam?

DanielleElmas [232]

Answer:

Steam always has more thermal energy than ice.

Explanation:

6 0

4 years ago

What is the mass of 40.34 x 10^23 H2 molecules at stp?

aev [14]

Every mol=6.22*10^23 <span>molecules and every mol of H2 Is 2 gram
40.34*10^23/6.22*10^23=6.48 or 6.5
6.5*2=13 gram
</span>

4 0

3 years ago

Read 2 more answers

A sample of unknown hydrate, AC-XH20, has a mass of 1.000 g before heating and a

KIM [24]

Answer:

The water of crystallization for the formula of the unknown hydrate is 2.

Explanation:

Mass of an unknown hydrate = 1.000 g

Molar mass of hydrate = 195.5 g/mol

MOles of unknown hydrate = $\frac{1.000 g}{195.5 g/mol}=0.00512 mol$

Mass of hydrate after heating = 0.781 g

Mass of water lost due to heating = x

$1.000 g = 0.781 g + x\\x = 1.000 g - 0.781 g = 0.219 g$

Moles of water lost = $\frac{0.219 g}{18.01528 g/mol}=0.0122 mol$

$AC.xH_2O+Heat\rightarrow AC+xH_2O$

1 Mole of hydrate has x moles of water and 0.00512 moles of hydrate has 0.0122 moles of water then we can write:

$\frac{1 }{x}=\frac{0.00512 }{0.0122 }\\x\approx 2$

The water of crystallization for the formula of the unknown hydrate is 2.

7 0

3 years ago

A box contains 104 gas molecules, 2500 of nitrogen and 7500 of argon in thermal equilibrium. The molecular weight of N2 is 28g/m

LekaFEV [45]

Answer : The temperature of this gas will be, 206.9 K

Explanation :

The expression for the kinetic energy per molecule of monoatomic gas (argon) is:

$K.E_{argon}=n_{argon}\times \frac{3}{2}\times K_BT$ ...........(1)

The expression for the kinetic energy per molecule of diatomic gas (nitrogen gas) is:

$K.E_{nitrogen}=n_{nitrogen}\times \frac{5}{2}\times K_BT$ .............(2)

The total kinetic energy of the molecule will be,

$K.E_{Total}=K.E_{argon}+K.E_{nitrogen}$

Now put all the expression in this, we get:

$K.E_{Total}=(7500)\times \frac{3}{2}\times K_BT+(2500)\times \frac{5}{2}\times K_BT$

$T=\frac{K.E}{17500\times K_B}$

Now put all the given values in this expression, we get:

$T=\frac{5\times 10^{-17}J}{17500\times (1.381\times 10^{-23}J/K)}$

$T=206.9K$

Therefore, the temperature of this gas will be, 206.9 K

8 0

4 years ago

How much of a 15.0M stock solution do you need to prepare 250ml of a 2.35ml hf solution?

Svetradugi [14.3K]

Using the relationship M1V1 = M2V2 where M1 and M2 are the molar concentrations (mol/L or mmol/ml) and V1 and V2 are the volumes of the solutions, we can arrive at the following answer for the given problem:

<span>15.0M (L of stock solution) = 2.35M (0.25L) *all volumes were converted to liters.

L of stock solution = (2.35*0.25)/15.0

Therefore, 0.0392L or 39.17 ml of stock solution is needed. </span>

3 0

3 years ago