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3 years ago

What is the most effective way to maintain good indoor air quality?

Chemistry

1 answer:

Masja [62]3 years ago

4 0

Answer:

close all doors and windows so the air stays inside

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What is the atomic mass of X ? Formula of the compound is XO3? Also identify the element X ? The molecular mass of XO3 is 80? (

djyliett [7]

Answer:

Explanation:

XO3

X + 3x16 = 80

x= 32 atomic mass for sulfur

SO3

6 0

3 years ago

150 mL of 0.25 mol/L magnesium chloride solution and 150 mL of 0.35 mol/L silver nitrate solution are mixed together. After reac

Murljashka [212]

Answer:

$0.175\; \rm mol \cdot L^{-1}$ .

Explanation:

Magnesium chloride and silver nitrate reacts at a $2:1$ ratio:

$\rm MgCl_2\, (aq) + 2\, AgNO_3\, (aq) \to Mg(NO_3)_2 \, (aq) + 2\, AgCl\, (s)$ .

In reality, the nitrate ion from silver nitrate did not take part in this reaction at all. Consider the ionic equation for this very reaction:

$\begin{aligned}& \rm Mg^{2+} + 2\, Cl^{-} + 2\, Ag^{+} + 2\, {NO_3}^{-} \\&\to \rm Mg^{2+} + 2\, {NO_3}^{-} + 2\, AgCl\, (s)\end{aligned}$ .

The precipitate silver chloride $\rm AgCl$ is insoluble in water and barely ionizes. Hence, $\rm AgCl\!$ isn't rewritten as ions.

Net ionic equation:

$\begin{aligned}& \rm Ag^{+} + Cl^{-} \to AgCl\, (s)\end{aligned}$ .

Calculate the initial quantity of nitrate ions in the mixture.

$\begin{aligned}n(\text{initial}) &= c(\text{initial}) \cdot V(\text{initial}) \\ &= 0.25\; \rm mol \cdot L^{-1} \times 0.150\; \rm L \\ &= 0.0375\; \rm mol \end{aligned}$ .

Since nitrate ions $\rm {NO_3}^{-}$ do not take part in any reaction in this mixture, the quantity of this ion would stay the same.

$n(\text{final}) = n(\text{initial}) = 0.0375\; \rm mol$ .

However, the volume of the new solution is twice that of the original nitrate solution. Hence, the concentration of nitrate ions in the new solution would be $(1/2)$ of the concentration in the original solution.

$\begin{aligned} c(\text{final}) &= \frac{n(\text{final})}{V(\text{final})} \\ &= \frac{0.0375\; \rm mol}{0.300\; \rm L} = 0.175\; \rm mol \cdot L^{-1}\end{aligned}$ .

6 0

3 years ago

Consider the statement below.

Vilka [71]

Answer:

Explanation:

Took the Edgenuity test

3 0

3 years ago

Calculate the rms speed of an oxygen gas molecule, o2, at 17.0 ∘c .

ludmilkaskok [199]

The RMS of O2 at 17 degrees is calculated as follows

RMs= ( 3RT/m)^1/2 where

R= ideal gas constant = 8.314
T= temperature= 17+273= 290 K
M= molar mass in KG = 32/1000= 0.032 Kg

Rms is therefore= sqrt (3x 8.314 x290/0.032 ) = sqrt( 226036.875

RMs=475.43

6 0

3 years ago

Read 2 more answers

17.g to mL<br> Density= 3.291g/mL

algol [13]

Density is defined as mass per unit volume
therefore density = mass ÷ volume

volume = mass÷density
volume in ml = 17 ÷ 3.291

4 0

3 years ago