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Natalka [10]
3 years ago
7

Type the correct answer in the box. Spell all words correctly. In which system are both energy and matter exchanged with the sur

roundings? In a(n) system both energy and matter are exchanged with the surroundings.
​

Chemistry
1 answer:
Anna11 [10]3 years ago
4 0

Answer:

open system

Explanation:

An open system is a system in which both energy and matter are exchanged with the surroundings.

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What is the net ionic equation of the reaction of MgSO4 with Pb(NO3)2?
NemiM [27]

Hey there!:

Write the molecular equation for the reaction of MgSO4 with Pb(NO3)2 :

MgSO4(aq) + Pb(NO3)2(aq) ---> Mg(NO3)2(aq) + PbSO4(s)

Write the total ionic equation  for the reaction :

Mg²⁺ (aq) + SO₄⁻² (aq) + Pb²⁺ (aq) + 2 NO₃⁻¹ (aq) + PbSO₄(s)

Therefore:

Cancel the spectator ions on both sides:

Pb²⁺ (aq) + SO₄⁻² (aq) ---> PbSO4(s)


Hope that helps!

4 0
3 years ago
Need a little help with chemistry :) <br> *if you don’t know, don’t answer*
Blizzard [7]

Answer:

1.33 moles

Explanation:

6 0
3 years ago
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Which of these compounds are molecular?<br> CBr4<br> FeS<br> P4O6<br> PbF2
olasank [31]

Answer:

I think it's answer is P4O6

I hope it's helpful for you...

8 0
3 years ago
If 97.3 L of NO2 forms measured at 35 C and 632 mm Hg. What is the percent yield?
enyata [817]
<span>a. Use PV = nRT and solve for n = number of mols O2. 
mols NO = grams/molar mass = ? 

 Using the coefficients in the balanced equation, convert mols O2 to mols NO2. Do the same for mols NO to mols NO2. It is likely that the two values will not be the same which means one is wrong; the correct value in LR (limiting reagent) problems is ALWAYS the smaller value and the reagent producing that value is the LR. 

b. 
Using the smaller value for mols NO2 from part a, substitute for n in PV = nRT, use the conditions listed in part b, and solve for V in liters. This will give you the theoretical yield (YY)in liters. The actual yield at these same conditions (AY) is 84.8 L. 

</span>and % will be 60%.
3 0
3 years ago
If 2.00 moles of H₂ and 1.55 moles of O₂ react how many moles of H₂O can be produced in the reaction below?
jekas [21]

Answer:

2 mol H₂O

Explanation:

With the reaction,

  • 2H₂(g) + O₂(g) → 2 H₂O(g)

1.55 moles of O₂ would react completely with ( 2*1.55 ) 3.1 moles of H₂. There are not as many moles of H₂, thus H₂ is the limiting reactant.

Now we <u>calculate the moles of H₂O produced</u>, <em>starting from the moles of limiting reactant</em>:

  • 2.00 mol H₂  * \frac{2molH_2O}{2mol H_2} = 2 mol H₂O
5 0
3 years ago
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