Answer and explanation:
1. To increases the accuracy of the measurement, the person should try to make sure the ruler is parallel to the object they are measuring. If they measure the object with the ruler not being parallel the measurement will end up larger then expected. To increase the precision the person must measure with the ruler in the same position each time.
2. A situation in which a set of measurements are precise but not accurate could be if a student measured an object at an incorrect angle many times, like the inaccurate measuring in the image above. All of the measurements would be inaccurate, but since they were all measured inaccuratly the same way, they will be precise.
3. An objects mass is defined as being the amount of matter in said object. An objects weight is defined as being the force exerted on an object by gravity. Although the man would weigh less on the Moon because there is less gravity, he still would not fit in his clothes because his mass has not changed.
Answer:
Molecules in order of decreasing rate of effusion:
![^1{H}^{35}Cl>^2H^{35}Cl>^1H^{37}Cl>^2H^{37}Cl](https://tex.z-dn.net/?f=%5E1%7BH%7D%5E%7B35%7DCl%3E%5E2H%5E%7B35%7DCl%3E%5E1H%5E%7B37%7DCl%3E%5E2H%5E%7B37%7DCl)
Explanation:
Mass of
gas= ![M_1= 36 g/mol](https://tex.z-dn.net/?f=M_1%3D%2036%20g%2Fmol)
Mass of
gas =![M_2= 38 g/mol](https://tex.z-dn.net/?f=M_2%3D%2038%20g%2Fmol)
Mass of
gas =![M_3= 37 g/mol](https://tex.z-dn.net/?f=M_3%3D%2037%20g%2Fmol)
Mass of
gas =![M_4= 39 g/mol](https://tex.z-dn.net/?f=M_4%3D%2039%20g%2Fmol)
According Graham's law:
'The rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas'.The equation given by this law follows the equation:
![\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20diffusion%7D%5Cpropto%20%5Cfrac%7B1%7D%7B%5Csqrt%7B%5Ctext%7BMolar%20mass%20of%20the%20gas%7D%7D%7D)
So, higher the molecular mass of the gas lower will be the effusion rate and vice versa.
Increasing order of molecular masses of the given gases:
![M_1](https://tex.z-dn.net/?f=M_1%3CM_3%3CM_2%3CM_4)
Decreasing order of effusion rate respective to gases:
![R_1>R_3>R_2>R_4](https://tex.z-dn.net/?f=R_1%3ER_3%3ER_2%3ER_4)
Molecules in order of decreasing rate of effusion:
![^{1}\textrm{H}^{35}Cl> ^{2}\textrm{H}^{35}Cl>^{1}\textrm {H}^{37}Cl>^{2}\textrm{H}^{37}Cl](https://tex.z-dn.net/?f=%5E%7B1%7D%5Ctextrm%7BH%7D%5E%7B35%7DCl%3E%20%5E%7B2%7D%5Ctextrm%7BH%7D%5E%7B35%7DCl%3E%5E%7B1%7D%5Ctextrm%20%7BH%7D%5E%7B37%7DCl%3E%5E%7B2%7D%5Ctextrm%7BH%7D%5E%7B37%7DCl)
HNO3 and H2SO4 are Arrhenius acids which will increase the concentration of H+ when dissolved in water.
KOH and Ca(OH)2 are Arrhenius bases that increase the concentration of OH- when dissociated in water.
The grams of oxygen that are required to produce 1 mole of H₂O is 16 g ( answer B)
<u><em> calculation</em></u>
2 CH₄ + 2NH₃ +3 O₂ → 2HCN + 6H₂O
step 1: use the mole ratio to find moles of O₂
from equation above the mole ratio of O₂: H₂O is 3:6 therefore the moles of O₂ = 1 mole x3/6 =0.5 moles
step 2: find mass of O₂
mass= moles x molar mass
from periodic table the molar mass of O₂ = 16 x2= 32 g/mol
mass O₂ = 0.5 moles x 32 g/mol = 16 g (answer B)
Answer:
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