Answer:
Stronium
Explanation:
It is a metal (and shows classic physical proerties). It also belongs to the second family, meaning it has two valence electrons.
Answer:
The equilibrium pressure of NO2 is 0.084 atm
Explanation:
Step 1: Data given
A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3.
Kp = 0.0118
Step 2: The balanced equation
NO( g) + SO3( g) ⇌ NO2( g) + SO2( g)
Step 3: The initial pressures
p(NO) = 0.86 atm
p(SO3) = 0.86 atm
p(NO2) = 0 atm
p(SO2) = 0 atm
Step 4: The pressure at the equilibrium
For 1 mol NO we need 1 mol SO3 to produce 1 mol NO2 and 1 mol SO2
p(NO) = 0.86 -x atm
p(SO3) = 0.86 -xatm
p(NO2) = x atm
p(SO2) = x atm
Step 5: Define Kp
Kp = ((pNO2)*(pSO2)) / ((pNO)*(pSO3))
Kp = 0.0118 = x²/(0.86 - x)²
X = 0.08427
p(NO) = 0.86 -0.08427 = 0.77573 atm
p(SO3) = 0.86 -0.08427 = 0.77573 atm
p(NO2) = 0.08427 atm
p(SO2) = 0.08427 atm
The equilibrium pressure of NO2 is 0.08427 atm ≈ 0.084 atm
Using accurate measurements, using pure chemicals and performing the reaction under the most ideal conditions is important to get a valuable percent yield.
<h3>How we calculate the percent yield?</h3>
Percent yield of any chemical reaction is define as the ratios of the actual yield to the theoretical yield of the product and multiply by the 100.
To get the high percent yield or actual yield of any reaction, we have to perform the reaction under ideal condition because if we not use the standard condition then we get the low rate of reaction. Reactants should be present in the pure form as impurity make unwanted products and reduce the productivity of main product and accurate amount of reactants also important for the spontaneous reaction.
Hence, options (a), (b) & (c) are correct.
To know more about percent yield, visit the below link:
brainly.com/question/8638404
C₄H₉OH + HBr = C₄H₉Br + H2O
Δmole of alcohol gives 1 mole of bromobutanol
HBr is in excess, so the yield of the product is limited by the alcohol
Wt. of 1 butanol = 18
Molar mass of the butanol = 74.12 g/mole
Moles of the alcohol = 1/74.12 = 0.01349 moles
So, moles of bromobutane = 0.01349 moles
Molar mass of C₄H₉Br = 137.018 g/moles
So, theoretical mass of bromobutane is = 0.01349 × 137.0.18
= 1.85 g
