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3 years ago

Plants use sunlight from the atmosphere during the process of

Chemistry

2 answers:

sergeinik [125]3 years ago

8 0

Answer:

Photosynthesis

Explanation:

Yeah

Nastasia [14]3 years ago

6 0

Answer:

photosynthesis

Explanation:

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Given the reaction:

Nadusha1986 [10]

Your answer will be B

8 0

3 years ago

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A 1.2516 gram sample of a mixture of caco3 and na2so4 was analyzed by dissolving the sample and completely precipitating the ca

Dennis_Churaev [7]

Answer:

0.009725 moles of H2C2O4

0.009725 moles CaCO3

Mass percentage = 77.77%

Explanation:

Step 1: The balanced equation

2MnO4- +5C2H2O4+6H+ →2Mn2+ +10CO2+8H2O

We can see that for 2 moles of Mno4- consumed , there is 5 moles of C2H2O4 needed and 6 moles H+ to produce 2 moles Mn2+, 10 moles of CO2 and 8 moles of H2O

Step 2: Calculate moles of MnO4-

Molarity = Moles/volume

Moles of Mno4- = Molarity of MnO4- * Volume of Mno4-

Moles of Mno4- = 0.1092M * 35.62 *10^-3 L

Moles of MnO4- = 0.00389 moles

Step 3: Calculate moles of H2C2O4

Since there is needed 5 moles of C2H2O4 to consume 2 moles of MnO4-

then for 0.00389 moles of MnO4-, there is 5/2 *0.00389 = 0.009725 moles of H2C2O4

Step 4: Calculate moles of CaCO3

moles of H2C2O4 = moles CaCO3, therefore, 0.009725 moles H2C2O4 = 0.009725 moles CaCO3

Step 5: Calculate mass of CaCO3

Molar mass of CaCO3 = 100.09 g/mole

Mass of CaCO3 = moles of CaCO3 * Molar mass of CaCO3

Mass of CaCO3 = 0.009725 moles * 100.09 g/mole = 0.9734 g

Step 6: Calculate percentage by weight of CaCO3

Mass of CaCO3 = 0.9734g

Mass of original sample = 1.2516g

Mass percentage = 0.9734/1.2516 *100% = 77.77%

6 0

3 years ago

A sample of a gas at 25°C has a volume of 150 mL when its pressure is 0.947 atm. What will the temperature of the gas be at a pr

sertanlavr [38]

Answer: The temperature of the gas at a pressure of 0.987 atm and volume of 144mL is $25.16^0C$

Explanation:

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 0.947 atm

$P_2$ = final pressure of gas = 0.987 atm

$V_1$ = initial volume of gas = 150 ml

$V_2$ = final volume of gas = 144 ml

$T_1$ = initial temperature of gas = $25^0C=(25+273.15)K=298.15K$

$T_2$ = final temperature of gas = ?

Now put all the given values in the above equation, we get:

$\frac{0.947\times 150}{298.15}=\frac{0.987\times 144}{T_2}$

$T_2=298.31K=(298.31-273.15)^0C=25.16^0C$

The temperature of the gas at a pressure of 0.987 atm and volume of 144mL is $25.16^0C$

4 0

2 years ago

Answer truthfully:))

Elina [12.6K]

Answer:

Formula: $Velocity \: V = f \lambda \\ Solution: = 5 \times 0.8 \\ = 4 \: {ms}^{ - 1}$

3 0

2 years ago

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Which planet formed near the sub where the solar system l’s temperatures were very high

Harrizon [31]

Answer:

Mars

Explanation:

Terrestrial or inner planets like Mars and Venus were formed near the Sun where the solar system's temperatures were very high.

4 0

3 years ago

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