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2 years ago

Sara has a red jacket. Which of the following models shows how Sara's jacket reflects and/or absorbs light?

Chemistry

2 answers:

just olya [345]2 years ago

7 0

I think it’s C. , C. Should be right because the red jacket is absorbing the light

Sonja [21]2 years ago

7 0

Answer:

answer choice c

Explanation:

the colors we see are the ones that are reflected off the object

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For each of the following acid-base reactions,

Sophie [7]

Answer: A. 3.28 g of HCl

B. 6.30 g of $HNO_3$

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} NaOH=\frac{3.65g}{40g/mol}=0.09moles$

$\text{Moles of} Ca(OH)_2=\frac{3.65g}{74g/mol}=0.05moles$

a) $HCl(aq)+NaOH(aq)\rightarrow H_2O(l)+NaCl(aq)$

According to stoichiometry :

1 mole of $NaOH$ require = 1 mole of $HCl$

Thus 0.09 moles of $NaOH$ will require= $\frac{1}{1}\times 0.09=0.09moles$ of $HCl$

Mass of $HCl=moles\times {\text {Molar mass}}=0.09moles\times 36.5g/mol=3.28g$

b) $2HNO_3(aq)+Ca(OH)_2(aq)\rightarrow 2H_2O(l)+Ca(NO_3)_2(aq)$

According to stoichiometry :

1 mole of $Ca(OH)_2$ require = 2 moles of $HNO_3$

Thus 0.05 moles of $Ca(OH)_2$ will require= $\frac{2}{1}\times 0.05=0.1moles$ of $HNO_3$

Mass of $HNO_3=moles\times {\text {Molar mass}}=0.1moles\times 63g/mol=6.3g$

6 0

1 year ago

How many grams of N2 are required to produce 100.0 L of NH3 at STP? 6.25 g

valentina_108 [34]

Given: N2, volume of 1L of NH3 at STP Required: Grams of N2 Solution: N2 + 3H2 -> 2NH3 Molar mass of N2 = 28g From the ideal gas equation PV = nRT n = PV/RT n = (1 atm)(100 L)/(0.08206 L-atm/mol-K)(273K) n = 4.46 mol of NH3 from the reaction, we need 2 moles of NH3 to get 1 mole of N2 4.46 mol NH3(1 mol N2/2 mol NH3) = 2.23 moles N2 2.23 moles of N2(28 g N2/1 mol N2) = 62.5g N2

5 0

2 years ago

A vessel of volume 100 cm3 contains 0.25 mol o2 and 0.034 mol co2 at 10.0c. Calculate the partial pressure of each component and

Artyom0805 [142]

Answer: The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.

Explanation:

According to the ideal gas equation:'

$PV=nRT$