Which of the following statements is true for ideal gases, but is not always true for real gases? Choose all that apply There are no attractive forces between molecules. Pressure is caused by molecule-wall collisions Replacing one gas by another under the same conditions, has no effect on pressure. Molecules are in constant random motion. Submit Answer Retry Entire Group 2 more group attempts remaining Solution 1. It is true that in real gases the attractive forces cannot be neglected. 2.In the real gas, the compressibility factor is not equal to 1. This implies that the molecule-wall collisions are in fact carry a prominent significance in projecting Pressure. 3. In ideal gases, the particle size is assumed to be constant and the interatomic spacing is considered to be almost negligible but it\'s not true in case of real gases..